Calculate the quantity of electricity required to liberate 0.1 mole of chlorine gas during electrolysis of molten sodium chloride.

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Aicharya · Accepted Answer

During electrolysis of molten NaCl , the following reaction takes place at anode: $2 \mathrm{Cl}^{-} \longrightarrow \mathrm{Cl}_2+2 \mathrm{e}^{-}$
1 mole of $\mathrm{Cl}_2$ is liberated with 2 moles of electrons. $\begin{aligned} & \therefore \quad 0.1 \text { mole of } \mathrm{Cl}_2 \text { will be liberated with } 0.2 \text { moles } \\ & \text { of electrons. } \end{aligned}$

Calculate the quantity of electricity required to liberate 0.1 mole of chlorine gas during electrolysis of…

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